name: key block: 1 foundations, measurement, and...scientific notation notes to put numbers in...
TRANSCRIPT
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Name: ______Key_____ Block:______
Unit 1
Foundations, Measurement, Safety and Matter Major Objectives: At the end of this unit, you should be able to:
1. Name and give the uses of ordinary laboratory equipment.
2. State the location of and proper use of our laboratory safety equipment.
IT IS REQUIRED THAT ALL STUDENTS WILL PASS A LAB TEST WITH A GRADE OF "B" OR
BETTER BEFORE PERFORMING ANY CHEMICAL LAB IN THIS COURSE.
3. Recognize the general steps scientists use in solving problems 4. Illustrate the scientific method 5. Show how numbers can be expressed in scientific notation. 6. Learn the metric system to measure length, volume, and mass 7. Learn to determine percent error 8. Learn to determine the number of significant figures in a calculated result 9. Learn how dimensional analysis can be used to solve various types of problems 10. Learn to determine density
Day Page # Description IC/HW Due Date Completed
?
1 X Signed Safety Agreement HW 9/2-3
1 X Signed Parent Letter HW
1 X Element Flash Cards HW
2 3‐8 Significant Figures IC/HW 9/4-5
3 X Diagnostic Math Test IC 9/8-9
3 9‐10 Equipment Scavenger Hunt IC
3 11‐13 Lab Safety Notes IC
4 X Lab Safety Test IC 9/10-11
Must get at least an 85%! 4 14‐15 Safety in the Lab Video IC
4 X Lab: Accuracy vs. Precision
(Long Pants and Closed Toed Shoes Required!)
IC/HW
4 14‐15 MSDS Challenge IC
4 16‐17 MSDS Explanation IC
4 X Physical/Chemical Properties Pre-
Lab “Quiz” HW
Due by the beginning of class Day 6
5 X QUIZ: Elements and Symbols IC 9/12-15
5 20‐22 SI Units and Dimensional
Analysis Notes IC 9/11-12
5 22‐24 Unit Conversion and Dimensional
Analysis Practice IC
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Day Page # Description IC/HW Due Date Completed
5 25‐26 Conversions and Dimensional
Analysis Homework Worksheet HW
5 X Unit Conversions HW HW Due: by 9/23/13
6 X
Lab: Physical and Chemical Properties
(Long Pants and Closed Toed Shoes Required!)
IC/HW
6/7 27‐30 Physical/
Chemical Properties and Changes Notes
IC
6 30 Chemical and Physical Properties Worksheet
IC/HW
6 X Polyatomic Ions HW HW Due by 9/27/13
7 31 Law of Conservation of Mass IC
7 32‐33 Classification of Matter
Worksheet HW
7 34‐37 Unit 1 Review HW
Learn the following symbols and the names of the elements which they represent. This is the first step in
learning to speak the language of Chemistry.
****QUIZ: Day 5 of Unit 1****
Ag Al Ar As Au B Ba Be Bi BrC Ca Cd Co Cr Cs Cu F Fe FrGa H He Hg I K Kr Li Mg MnMo N Na Ne Ni O P Pb Ra RbRn S Sb Se Si Sn Sr Xe Zn ClW Y
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Unit 1: Significant Figures and Scientific Notation
Scientific Notation Notes
To put numbers in scientific notation:
1. Place the decimal after the ______first number moving left to right____.
2. Rewrite the number and multiply it by 10x.
3. Count the number of spaces you moved the decimal. This number is x (the exponent for the ten).
4. If the original number was less than one, the exponent is ___negative___.
Practice Problems
5) 0.000 000 000 000 615 g 6.15 x 10‐13 g
6) 98 000 000 000 m 9.8 x 1010 m
7) 0.000 104 s 1.04 x 10‐4 s
8) 407 302 000 000 000 Pa 4.07302 x 1014 Pa
9) 4.38 x 10‐7 km 0.000 000 438 km
10) 1.89 x 104 L 18 900 L
11) 7.4 x 10‐4 g 0.000 74 g
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Percent Error Notes Accuracy, Precision, and Error
Accuracy – the __closeness____of a measurement to the__true___ value of what is being measured
‐ accuracy can be determined by _one_ measurement
‐ depends on the _quality_of the _____measurement___
Precision – describes the closeness, or ___reproducibility___, of a set of measurements taken under
the _same_ conditions
‐ precision is determined by ___more than one _measurement
‐depends on the __skills___of the person measuring
Accepted (or theoretical) value – a quantity used by general agreement of the scientific community
Experimental (or actual) value – a quantitative value measured during an experiment
Error – the __percent error___ between the__actual ___ value and the__experimental__ value
Error =
Error = E – A E = Experimental value A= Accepted value
Percent error = the percent that a measured value differs from an accepted value
| |
Example: Peter measured the volume of a 2 liter bottle of soda. The actual volume of the soda was 1.87 Liters.
What is the percent error of the volume of soda?
%E = │ E — A│ x 100 =
A
%E = │ 1.87 L — 2.00L│ x 100 = 6.5%
2.00 L
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Significant Figures
The Atlantic/Pacific Rule for Determining Significant Figures 1) look for the presence, or not, of a decimal point - this will tell you which side to start counting from - Pacific: left - Atlantic: right 2) if there is a decimal point you start counting from the left side of the number - starting from the very left side of the number, look for the first non-zero number - count the first non-zero number and every number (0-9) after that
- example: 0.00010 - because there is a decimal point, we start from the left side of the equation L0.00010, and
look for the first non-zero number 0.00010
- count that number and every number after that regardless of what the number is (0-9) - in this case there are 2 significant figures
- 0.00010 3) if there is not a decimal point you start counting from the right side of the number - starting from the very right side of the number, look for the first non-zero number - count the first non-zero number and every number (0-9) after that
- example: 721000 - because there is a decimal point, we start from the right side of the equation 7210007, and
look for the first non-zero number
721000 - count that number and every number after that regardless of what the number is (0-9) - in this case there are
PACIFIC (Present)
ATLANTIC (Absent)
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Significant Figures: All exact digits of a measurement plus one estimated digit.
Brief determination of the number of significant digits
Rule #1: All non‐zero numbers are significant 732 g
Rule #2: Any zero’s between non‐zero numbers are significant 301 cm
Rule #3: If there is a decimal point, any zero’s to the right of the last non‐zero are significant
a. 320. kg 3 significant figures
b. 320 kg 2 significant figures
c. 0.70 m 2 significant figures
d. 0.070 m 2 significant figures
Rule #4: Any number that is used to count things or is a direct conversion has infinite significant
figures.
a. 45 desks infinite significant figures
b. 60 s = 1 minute infinite significant figures
c. 10 pennies = 1 dime infinite significant figures
d. 4 beakers infinite significant figures
Helpful Hint
If the value _is written__ with a visible decimal point, then go to the___left__ end of the value.
Moving right, find the first non‐zero number; count it and every number to the right.
If the decimal point is __Present__you start on the __Pacific___side of the equation.
⟶0.0012040 5 significant figures
If the value is not ___written_____ with a visible decimal point, go to the ___right_end of the value.
Moving to the left find the first non‐zero number; count it and every number to the left.
If the decimal point is __absent__you start on the ___Atlantic__side of the equation.
7201000 ⟵ 4 significant figures
Rounding off numbers
Rule #1: If the number after the number to be rounded is less than 5, round down.
Rule #2: If the number after the number to be rounded is greater than or equal to 5, round up.
In a series of calculations, carry extra digits through to the final result and then round off. This means that you should carry all of the digits that show on your calculator (or most of them) until you arrive at your final answer and then round off.
Note: Don’t forget significant zeros when writing in scientific notation (ex: 20.0 is 2.00 x 10). Do not
write INsignificant zeros when writing in scientific notation (ex: 6 000 000 is 6 x 106, not 6.000 000 x
106 – this number would have 7 sig figs).
Addition and Subtraction
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Rule: Complete the desired calculation and then round off the answer to the number of decimal
places as the value from the problem with the ________ NUMBER OF DIGITS _ THE DECIMAL.
a) 12.72 34.1 + 0.463
47.283 47.3
all numbers are significant to the tenths place.
b) 900 370 + 101.037
1,371.037 1,371
All numbers are significant to the Left of the decimal_ place.
c) 790. 330 + 54.8
1,174.8 1,175
All numbers are significant to the __ left of the decimal__ place. Multiplication and Division
Rule: Complete the desired mathematical calculation and then round off the answer to the same
number of significant figures as the value from the problem with the __least__ NUMBER OF
SIGNIFICANT FIGURES.
34.91 x 0.0053 = 0.185023 Rounds to 0.19 four two two sig figs sig figs sig figs
Because 0.0053 has only two significant figures, it limits the answer to two significant figures.
3. 102 ÷ 0.0097 = = 319.7938144 Rounds to 320 4 sig figs 2 sig figs
Combination of operations Complete mathematical calculations in correct order and use correct number of significant figures after
each step.
Example: (5.2 – 0.2) x 7.00 x 1.00 = 35.00
The difference of 5.2 and 0.2 is 5.0 which is precise to the nearest tenth and has 2 sig. figs.
Since 7.00 and 1.00 have 3 sig. figs. The least number of sig figs in the multiplication
operation is 2 from the 5.0 difference. The final answer has 2 sig figs. Answer = 35
Pacific – Atlantic Rule
If the decimal is PRESENT, start on the PACIFIC side or ____left to right___.
14.020 0.00235 1.04 * 105
If the decimal is ABSENT, start on the ATLANTIC side or _____right to left_____.
7300200 1200 839
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Significant Figures and Scientific Notation Worksheet
Underline the significant
figures in the following
measurements and put the
number in scientific notation:
1. 0.00325 m 3.25 x 10‐3 m
2. 12500 s
1.25 x 104 s
3. 304.00 g 3.0400 x 102 g
4. 0.00256 kg
2.56 x 10‐3 kg
5. 0.0030600 J
3.0600 x 10‐3 J
6. 6.0250 Mm
6.0250 x 100 Mm
Round the following measurements
to the requested number of
significant figures and put the
number in scientific notation:
1. 0.003256 m 2 sig. figs.
3.3 x 10‐3 m
2. 564025000 g 3 sig. figs.
5.64 x 108 g
3. 78265 ns 1 sig. fig.
8 x 104 ns
4. 0.236578 Pa 4 sig. figs.
2.366 x 10‐1 Pa
5. 0.008596 ng 3 sig. figs.
8.60 x 10‐3 ng
6. 15.349 mg 4 sig figs.
1.535 x 101 mg
Put the following
measurements in scientific
notation and put the number
in scientific notation:
1. 0.000000586 m 5.86 x 10‐7 m
2. 5620000 g
5.62 x 106 g
3. 85000 L
8.5 x 104 L
4. 0.00236 km
2.36 x 10‐3 km
5. 25640000000 Pa
2.564 x 1010 Pa
6. 0.000001524 s
1.524 x 10‐6 s
Perform the following calculations and write the answer with the appropriate number of sig figs AND in
scientific notation.
1. 6.23 x 106 kL + 5.3 x 106 kL 2. 7.525 x 105 kg ‐ 5.43 x 102 kg
1.2 x 107 kL 7.52 x 105 kg
3. 4.8 x 105 km x 2.02 x 103 km 4. 8.45 x 102 cm3 ÷ 7.901 x 103 cm3
9.7 x 108 km 1.07 x 10‐1 cm3
5. 2.45 x 10‐15 J ÷ 3.4 x 10‐19 J 6. 20.05 x 10343 – 15.9 x 10341
7.2 x 103 J 19.9 x 10343
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Name______________________________
Partner(s): ______________________________________________
Equipment Scavenger Hunt
Find the following items and write the location in the space provided. If there is a number next to an item, that
is how many locations you must find. Use descriptive words when describing the areas of the classroom, and
tell what the item is next to.
Item Location
Eye Wash ___It is the back of room near rear door under shower______
Exits (2) The door in the front of the room and the door in the back of the room_
Fire Blanket _The rear of the room between the fume hoods and cabinet__________
Fire Extinguisher ___The front of the room next to the classroom door_________________
Fume Hood ___The rear of the classroom in the middle of the room_______________
Goggle Cabinet ___Back of room next to fume hood and fire blanket _______
Hole Punch ____On Mr. Buchanan’s cart_____________________________________
In Bins ______________________________________________________
Out Bins ______________________________________________________
Pencil Sharpener __Front of classroom next to door________________________________
Recycling Bin __Both are in the front of classroom next to door ___________________
Safety Shower __Rear of classroom between fume hood and door, over eye wash______
Sign In/Out __Front of classroom next to door on table________________________
Wastebasket (3) __Front of classroom next to door, under board and in the back next to goggle
cabinet__
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Equipment Scavenger Hunt:
On the lab bench there is equipment laid out for you to identify. While you may not know all of the equipment,
try your best to identify all of it. Write the letter on the equipment next on the line next to the name.
1. Beaker ______
2. Beaker Tongs ______
3. Bunsen Burner ______
4. Buret ______
5. Buret Clamp ______
6. Clay Triangle ______
7. Crucible ______
8. Crucible Tongs ______
9. Erlenmeyer Flask ______
10. Evaporating Dish ______
Map of Key Safety Equipment in the Room Draw the following pieces of safety equipment
in the room map below. Be sure to label all of
the items below using their designated letter.
A. Eye Wash B. Exits (2) C. Fire Blanket D. Fire Extinguisher E. Fume Hood F. Goggle Cabinet G. Safety Shower H. Window I. Lab Stations
11. Forceps ______
12. Funnel ______
13. Graduated Cylinder ______
14. Striker ______
15. Ring Clamp ______
16. Test Tube ______
17. Volumetric Flask ______
18. Wash Bottle ______
19. Watch Glass ______
20. Wire Gauze ______
Teacher’s Desk
Door
Exit
D E O X O I R T
Fire Blanket FUME
HOODS
Goggle Shower
Eye‐Wash
W
I
N
D
O
W
S
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Lab Safety Notes
__Goggles_______ should be worn at all times when in the lab.
___Short pants/ dresses / floppy clothes______ can never be worn in the lab. All shoes
must have ________closed toes___________________.
If your lab partner is on fire, you should ________wrap him in the fire blank_______
____and notify the teacher asap_________________________________.
If you get chemicals in your eyes you should use the eye wash station for _15/20__ minutes.
The _______fume hood_____ is used to remove noxious fumes and vapors.
If you spill a large amount of chemical on you, you should ______________
_______________safety shower______________________.
When heating a test tube, you should always ______point the mouth (opening) of the
testtube away from yourself and others___.
Wafting is a method of smelling chemicals by _______moving your hand over the
chemicals but without directly inhaling the fumes___________.
You should never __eat__ or ____drink___ in the lab.
You must complete the ____prelab___ if you want to participate in the lab. You MUST read
the __MSDS sheet___ before you enter the lab.
Contact lenses should ___not_____ be worn in the lab area.
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MSDS (Material Safety Data Sheet) Challenge
Determine the identity of the unknown chemical that was used in the demonstration.
1. What factors can be used to determine which chemical was used?
2. Where can you find flammability information on the MSDS Sheet? Determine which chemicals are flammable from the MSDS Sheets and fill in the Flammability Column on the table below.
3. Fill in the following table with the information from the MSDS sheets given:
Chemical Physical Properties FlammabilityMelting Point
Soluble in Water?
Specific Density
Cyclohexane
Ethylene Dichloride
Glycerin
Isopropyl Alcohol
Succinic Acid
Water
4. What is the identity of the unknown substance? Explain
OMIT
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Select of the substances from the MSDS Sheets and answer the following questions (Do NOT select
water):
5. Chemical Identity
6. What may happen if you inhale your substance?
7. What chemicals should not be stored with your chemical?
8. How do you clean up a spill of your chemical?
9. List any special protection or precautions.
OMIT
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“Accident at Jefferson High” Safety Video Questions Complete the following questions individually as you watch the video:
1. Accidents always occur because of __PEOPLE’S MISTAKES (goofing off)______
2. List some of the typical hazards in a science lab.
__Acids ( Nitric)______Fires___________________________
__Spills________ Mixing Chemicals incorrectly______
3. List several possible accidents which may occur during a laboratory activity.
___Drinking and Eating in Lab (never) _____________________________
__ Not following proper procedures (lighting Bunsen burners)__________
4. List some things that should be done to prepare for a lab.
__Be alert and proceed with caution___________
___Tie back hair____________________________
___Remove jewelry__________________________
___Wear long pants and closed toe shoes________
5. To dilute an acid, always add the acid __into water______
6. Never __taste__ or __directly smell___ or ___touch___ chemicals.
7. How can one avoid “mix‐ups”? ___Read labels and double check labels_
8. Acid spills are best neutralized with __a weak base (sodium carbonate solution) .
9. Base spills are best neutralized with _a weak acid (vinegar)____
10. How would you treat an acid or base spill on the skin or into the eyes?
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Skin: _Wash it off immediately with lots of water______
Eyes: _Rinse your eyes in the eyewash for approximately 15/20 minutes._______
11. When lighting the burner, always turn on the gas after lighting your match and hold it over
the burner__
12. What do you use to tell the difference between hot and cool glass?
___Use the back of your hand to hold over the hot object____________
13. List some safety considerations for heating liquids in a test tube.
Face opening of test tube away from yourself and others___
Move the test tube up and down in flame to heat all the content equally_
14. Flammable liquids should be extinguished by __USING A FIRE EXTINGUISHER__
Answers to Lt. Grumman‛s Safety Test (True/False)
1. True 8. True
2. False 9. True
3. False 10. True
4. True 11. False
5. False 12. True
6. True 13. True
7. True 14. False
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Section I - Product Identification:
Manufacturer's Name: The manufacturer of the product is listed along with the manufacturer's address.
Emergency Telephone Number: The telephone number of people other than the manufacturer who may provide information for a chemical emergency; a spill, explosion, fire, etc.
Chemical Name and Synonyms: Chemical name of the material, if it is a single element or compound, along with other terms for the substance.
Trade Name and Synonyms: The name the product is sold by along with other terms for the formulation.
Chemical Family: General class of compounds to which a material belongs (e.g. ether, mineral acid, ketone, etc.).
Formula: Formula for the number and types of atoms contained in the substance if it is a single element or compound.
Section II - Hazardous Ingredient Information:
Hazardous Ingredients: Listed by chemical name in one of three divisions (paints, preservatives and solvents; alloys and metallic coatings, or hazardous mixtures of other liquids, solids, or gases) unless the product is a bona fide trade secret.
Percentage: Percent by weight or volume of each ingredient.
PEL: Term used by the Occupational Safety and Health Administration (OSHA) to express the legal airborne concentration of a material to which persons can be exposed day after day. Usually stated in parts per million (ppm) or milligrams per cubic meter (mg/M3).
TLV: Term used by the American Conference of Governmental Hygienists (ACGIH) to express the airborne concentration of a material to which nearly all persons can be exposed day after day, without adverse health effects.
Section III - Physical Data:
Boiling Point: Temperature at which a liquid changes to a vapor at a given pressure, usually stated in of at one atmosphere pressure. For mixtures, the initial boiling point or boiling range may be given.
Vapor Pressure: Pressure exerted by a vapor above its own liquid in a closed container, usually stated in millimeters of mercury (mm of Hg) at 20oC (unless stated otherwise).
Vapor Density: Relative density or weight of a vapor or gas compared to an equal volume of air. Air is rated as 1.0.
Solubility in Water: The amount of a substance which can be dissolved in a given volume of water. Expressed usually in terms of milligrams per liter or in general terms such as "negligible."
Appearance and Odor: Brief description of the substance at normal room temperature and atmospheric conditions (e.g. viscous, colorless liquid with an aromatic hydrocarbon odor).
pH: An expression of the acidity or alkalinity of an aqueous solution by the logarithm of the reciprocal of the hydrogen ion concentration.
Specific Gravity: Weight of a volume of substance to an equal volume of water. A ratio of less than one means the material is lighter than water and vise versa.
Percent Volume by Weight: Percent of a liquid or solid (by volume) that will evaporate at an ambient temperature of 70oF.
Evaporation Rate: Rate at which a material is converted to the vapor state at any given temperature and pressure.
Section IV - Fire and Explosion Hazard Data:
Flash Point and Method Used: Lowest temperature at which a liquid will give off enough flammable vapor to ignite.
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Flammable Limits: Range of concentrations over which a flammable vapor mixed with air will flash or explode if an ignition source is present.
Extinguishing Media: Fire-fighting material for use on substance that is burning, Fire-fighting material should be indicated by its generic name (e.g. water, foam, dry chemical, etc.).
Special Fire Fighting Procedures and Precautions: Listing of certain fire-fighting materials unsuitable or unsafe to use on the burning substance. Also, a listing of special handling procedures and personal protective equipment.
Unusual Fire and Explosion Hazards: Hazards which might occur from overheating or burning of substance, including any chemical reactions or changes in chemical form or composition. Also, any special hazards which may need to be considered while extinguishing a fire.
Section V - Health Hazard Data:
Threshold Limit Value: Explained previously in Section II.
Effects of Overexposure: Covers immediate (acute) and long-term (chronic) effects of overexposure to the substance. May include information from human experience and animal tests. Toxicity data may also be provided in the form of average lethal dose or concentration (LD50 or LC50, respectively).
Emergency and First-Aid Procedures: Emergency information and first aid instructions for treatment of acute inhalation, ingestion, and skin or eye contact.
Section VI - Reactivity Data:
Stability: Indication of whether the substance is susceptible to dangerous decomposition and under what conditions it might occur.
Conditions to Avoid: Conditions which may cause hazardous consequences or damage to the substance (e.g. heat, shock, cold, light).
Incompatibility: Common materials or contaminants with which the specific substance may come in contact and release large amounts of energy, flammable vapor or gas, or produce toxic vapor or gas.
Hazardous Decomposition Products: Hazardous materials that may be produced in dangerous amounts if the substance is exposed to burning, oxidation, heating or allowed to react with other chemicals.
Hazardous Polymerization: Polymerization is a chemical reaction in which two or more small molecules combine to form larger molecules that contain repeating structural units of the original molecules. A hazardous polymerization is an unintended and uncontrolled polymerization reaction that may create a great deal of heat and may release a hazardous substance.
Section VII - Spill or Leak Procedures:
Spill and Leak Procedures: Immediate steps to be taken to assure safety to people and property in the event of a spill or leak of the substance including equipment and personal protective equipment. Methods for control and clean-up are described.
Waste Disposal Method: May describe a method for disposing of excess, used, or spilled material.
Section VIII - Special Protection Information:
Respiratory Protection: Requirements for respiratory protection should ventilation recommendations not be feasible.
Ventilation: Type of ventilation, if needed when working with the substance.
Protective Gloves: The appropriate gloves, if needed, to prevent hand contact (e.g. rubber, vinyl, neoprene).
Eye Protection: Type of eye protection device to be worn when working with the substance.
Other Protective Equipment: Additional protective measures or equipment recommended when working with the substance (e.g. apron, boots, glove box)
Section IX - Special Precautions:
Precautions to be Taken in Handling and Storage and Other Precautions: Describes additional precautions to be considered or may give special emphasis to information or warning stated in other sections of MSDS.
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SI Unit Notes
Dimension Base Unit Symbol
Length/Distance Meter m
Mass kilogram kg
Temperature Kelvin K
Volume Decimeter cubed and Liters dm3 and L
Time second s
Energy Joule J
Speed meter per second m/s
Frequency 1/second = Hertz Hz
Density Gram/centimeter3 g/cm3
Pressure Pascal Pa
Temperature: Celsius and Kelvin
Equal Units of Volume: 1 cm3 = 1 mL 1 dm3 = 1 L Density: g/mL or g/cm3
Theory Law
‐ Explains a scientific Relationship‐ Must be testable ‐ Must be falsifiable
‐ Cannot be proven true, can be proven wrong
‐ Can be modified to incorporate new data ‐ Can be used to make accurate predictions
‐State a scientific relationship‐must be verified by data
‐ Modified as conflicting data is gathered
‐Can be used to make accurate predictions ‐Can be expressed mathematically
Observation: The act of gathering specific information using the 5 senses.
Inference: The act or process of deriving logical conclusions from premises known or assumed to be true or the act of reasoning from factual knowledge or evidence.
Hypothesis: A tentative explanation for a question, testable through experiments
Accuracy: Accuracy refers to the correctness of a single measurement. Accuracy is determined by comparing the measurement against the true or accepted value.
Precision: Precision refers to how well experimental data and values agree with each other in multiple tests.
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SI Unit Prefixes
Prefix Symbol Meaning
Mega M 106
Kilo k 103
Deca D 101
Base ‐‐ 100
deci d 10‐1
centi c 10‐2
milli m 10‐3
micro µ 10‐6
nano n 10‐9
pico p 10‐12
You must memorize these prefixes, symbols and meanings! Remember, when you are dividing exponents, you subtract.
103 ÷ 106 = 10‐3 because (3 – 6 = ‐3)
Remember, when you are multiplying exponents, you add.
102 x 103 = 105 because (2 + 3 = 5)
Steps for SI Conversions
1. Write down the starting measurement
2. Put the units of the starting measurement into the denominator to cancel
3. Put units you want on the top
4. Put a 1 with the larger unit
5. Determine relationship between the two units (MEMORIZE prefix chart) by finding the absolute value of the difference in exponents.
6. Solve. Cancel units. If exponent jumps the line then change the sign (105=1/10‐5) 7. If needed put the number into scientific notation.
SI Conversions Example 1:
63 200 centiliters microliters
63,200 centiliters 104 microliters = 6.32 x 108 microliters
1 centiliters
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SI Unit Conversions Practice:
1. 89.3 kilometers nanometers
89.3 kilometers 1012 nanometers = 8.93 x 1013 nanometers
1 kilometers
2. 5.32x108 picograms milligrams
5.32x108 picograms 1 milligrams = 5.32 x 10‐1 milligrams or 0.532 mg
109 picograms
3. 26.60 millipascals megapascals
26.60 millipascals 1 megapascals = 2.660 x 10‐8 megapascals
109 millipascals
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DIMENSIONAL ANALYSIS NOTES:
If light from the sun takes 8.11 minutes to get to the Earth, how far away is the sun in km? (speed of
light is 3.0x108m/s and there are 1000 m in one km)
1. Identify the values in the problem, include units
8.11 minutes 1000 m in one km
3.0x108m/s
2. Start with the value with only one unit
8.11 minutes
3. Put that starting unit into the denominator to cancel units out
8.11 minutes
minutes
4. Find the value OR conversion to a given value with the same unit and place it into the problem
8.11 minutes 60 seconds
1 minutes
5. Repeat until you get to the desired units, cross out units which cancel
8.11 minutes 60 seconds 3.0x108 meters 1 Kilometers
1 minutes 1 seconds 1000 meters
6. Solve and put into correct scientific notation (multiply numerator and divide denominator)
DIMENSIONAL ANALYSIS PRACTICE PROBLEM:
If you live 3.2 miles from your best friend and the speed limit is 25 miles/hour, how many seconds will it
take you to drive from your house to your friend’s house?
= 460.8 seconds
460 seconds
3.2 miles 1 hour 60 minutes 60 seconds
25 miles 1 hour 1 minutes
= 1.46 x 108 km
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SI Unit Conversions Practice 1. Convert 0.0036 g to mg
0.0036 g 1000 mg = 3.6 mg
1 g
2. Convert 8.9 x 10‐8 s to ps
8.9 x 10‐8 s 109 ps = 89 ps
1 s
3. Convert 8200000 nPa to MPa
8200000 nPa 1 MPa = 8.2 x10‐9 MPA
1015 nPa
4. Convert 3.26 L to cm3
3.26 L 1000 cm3 = 3.26 x103 cm3 or 3260 cm3
1 L
5. Convert 0.0012 cm3 to mL
0.0012 cm3 1 mL = 0.012 mL
1 cm3
6. Convert 0.29 L to cm3
0.29 L 103 cm3 = 290 cm3
1 L
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Dimensional Analysis Practice Problems:
Remember ‐ The numbers in conversion factors are considered to be exact. Be sure to include units where appropriate, and round your answers according to the number of digits in the original problem.
1. Convert 2.44 L to cm3
2.44 L 103 cm3 = 2440 cm3
1 L
2. Convert 45 654 mg to kg
45 654 mg 1 kg = 0.045654 kg
106 mg
3. Convert 4.7 km/hr to m/s
4.7 km 103 m 1 hr = 1.305556 m/s
1 hr 1 km 3600 s
1.3 m/s
4. Convert 4.00 g/cm3 to kg/dm3
4.00 g 1 kg 103 cm3= 4.00 kg/dm3
1 cm3 103 g 1 dm3
5. Convert 6.72 dm3/s to L/min
6.72 dm3 1 L 60 s = 2803.2 L/min
1 s 1 dm3 1 min
2.80 x 102 L/min
6. Convert 0.0598 mg/cm3 to g/cm3
0.0598 mg 1 g = 5.98 x 10‐5 g/cm3
1 cm3 103 mg
7. Convert 2.7 dm3 to mL
2.7 dm3 103 mL = 2.7 x 103 mL
1 dm3 2,700 mL
8. Convert 0.90 kg/cm3 to mg/ cm3
0.90 kg 106 mg = 0.90 x106 mg/mm3
1 cm3 1 kg
9.0 x 105 mg/cm3
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Dimensional Analysis Word Problems Practice 1. You want to earn $600.00 to buy a new bicycle. You have a job that pays $8.75/hour, but you
can work only 3 hours/day. How many days before you will have enough to buy the bike?
$600.00 1 hr 1 day = 22.85714 days or 23 days
$8.75 3 hr
2. Someone that never learned dimensional analysis went off to work at a fast food restaurant for the past 35 years wrapping hamburgers. Each hour you wrap 184 hamburgers. You work 8 hours per day. You work 5 days a week. You get paid every 2 weeks with a salary of $840.34. How many hamburgers will you have to wrap to make your first one million dollars?
$1,000,000 2 weeks 5 days 8 hrs 184 hmbrgrs = 17516719.42 hmbrgrs
$840.34 1 week 1 day 1 hr
= 17,500,000 hmbrgrs
3. In 1973 the Emergency Highway Energy Conservation Act instituted a National Maximum Speed Law of 55 mph. How many minutes would it take to travel 16 kilometers? (1 mile = 1.6093 km)?
16 km 1 mile 1 hr 60 min = 10.84604825 min
1.6093km 55 mile 1 hr
11 min
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Conversions and Dimensional Analysis Homework Worksheet
Metric Conversions:
1. Convert 2.5 cm to m 2.5 cm 1 m = 2.5 x 10‐2 m 100 cm = 0.025 m
2. Convert 3.87 m to cm
3.87 m 100 cm = 3.87 x 102 cm 1 m
3. Convert 25 mm to m
25 mm 1 m = 2.5 x 10‐2 m 1000 mm
4. Convert 105 m to mm
105 m 103 mm = 1.05 x 105 m 1 m
5. Convert 1.8 km to m
1.8 km 103 m = 1.8 x 103 m 1 km
6. Convert 2.38 x 102 m to km 2.38 x 102 m 1 km = 2.38 x 10‐1 m 1000 m
7. Convert 40.0 m to mm 40.0 m 1000 mm = 4.00 x 104 cm 1 m
8. Convert 8.0 cm to mm
8.0 cm 10 mm = 80. mm 1 cm
9. Convert 0.02 mm to cm 0.02 mm 1 cm = 0.002 cm 10 mm
10. Convert 57.2 mm to km
57.2 mm 1 km = 5.72 x 10‐5 km 106 mm
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Dimensional Analysis Problems:
11. Convert 2.05 x 105 seconds into years.
2.05 x 105 s 1 hr 1 day 1 year = 6.50 x 10
‐3 yrs
3600 s 24 hr 365 days
12. Traveling at 65 miles/hour, how many minutes will it take to drive 125 miles to San Diego?
125 miles 1 hr 60 min = 115.3846154 min ≈ 120 min
65 miles 1 hr
13. Convert 50 years into seconds. Express your answer in scientific notation.
50 years 365 days 24 hrs 60 min 60 s = 1.576800000 x 109 s ≈ 2 x 109 s
1years 1 day 1 hr 1 min
14. Traveling at 65 miles/hour, how many feet can you travel in 22 minutes? (1 mile = 5280 feet)
22 min 1 hr 65 miles 5280 ft = 125,840 ft ≈ 130,000 ft = 1.3 x 105 ft 60 min 1 hr 1 mile
15. In Raiders of the Lost Ark, Indiana Jones tried to remove a gold idol from a booby‐trapped pedestal. He replaces the idol with a bag of sand. If the idol has a mass of 2.00 g, how many liters of sand must he place on the pedestal to keep the mass sensitive booby‐trap from activating? (Density of sand is 3.00 g/cm3)
2.00 g 1 cm3 1 L = 6.67 x 10‐4 L
3.00 g 1000 mL
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Physical/Chemical Properties and Changes Notes
What is matter?
Matter is the term for any type of material. Matter is anything that has mass and takes up space. The word is sometimes used to refer to a pure substance.
Physical Properties: Properties of a substance that can be measured without changing the
chemical nature of the substance.
o Examples: Color, Smell, Freezing point, Boiling point, Melting point, Magnetism, Opacity,
Viscosity and Density
o Intensive Properties: are ___Independent__ of the amount of matter present.
Examples: Temperature, color, hardness, melting point, boiling point, pressure, molecular weight, and density. Because intensive properties are sometimes characteristic of a particular material, they can be helpful as clues in identifying unknown substances.
o Extensive Properties: are ____ Dependent ____ on the amount of matter present.
Examples: Mass, volume, length, and total charge.
Chemical Properties: Properties of a substance that cannot be measured without changing the
chemical nature of the substance.
o Examples: Combustion and reactivity with water
Physical Changes: Changes that do not alter the chemical composition of a substance.
o Examples: Physical changes are concerned with energy and states of matter. A
physical change does not produce a new substance. Changes in state or phase (melting, freezing, vaporization, condensation, sublimation) are physical changes. Examples of physical changes include crushing a can, melting an ice cube, and breaking a bottle.
Chemical Changes: Changes that alter the chemical composition of a substance.
o Examples: Chemical changes take place on the molecular level. A chemical change produces a new substance. Examples of chemical changes include combustion (burning), cooking an egg, rusting of an iron pan, and mixing hydrochloric acid and sodium hydroxide to make salt and water.
Indications of a chemical change: Change in odor Change in color Energy given off or absorbed Formation of a precipitate
Formation of a gas
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The Four Aristotelian Elements
Western chemistry grew up around old alchemical ideas of Earth, Air, Fire, and Water – the so called Aristotelian elements – a concept that originated with the ancient Greeks and others.
Matter Notes
Solid Liquid Gas
Vapor: is not the same as gas. Vapor refers to the gaseous phase of a substance that is a liquid
or solid under standard conditions.
Alloy: A metallic solid solution composed of two or more elements.
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Solid Liquid Gas
Plasma: high temperature, low pressure; electrons separate from nucleus; most common in
the universe
Elements, Compounds, Mixtures and Solutions
Elements: a pure substance that is made up of only one type of atom and cannot be broken down by physical or chemical means.
Examples: There are 115 known elements presently, out of which only 91 occur naturally. The remaining elements have been produced artificially by nuclear scientists in the laboratory using particle accelerators.
Compounds: a combination of two or more different elements that are combined chemically. o Examples: The smallest unit of a compound, known as a molecule, or a formula unit,
is composed of atoms of the constituent elements. A compound is represented by a chemical formula which indicates one molecule (formula unit) of the compound containing atoms of its elements.
Mixture: a combination of two or more pure substances in which each pure substance retains its physical properties.
Examples: Milk, Salt water
o Homogeneous mixture: Mixtures in which the composition is uniform throughout. Also called a SOLUTION. Examples:
1. Blood 2. Sugar solution when sugar is completely dissolved. 3. Mixture of alcohol & water 4. A glass of orange juice 5.salty water (where the salt is completely dissolved) 6.brewed tea or coffee
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o Heterogeneous mixture: Mixtures in which the composition is not uniform throughout. You can distinguish the different parts. Examples:
1. Oil & water. 2. Soil sample 3.sandy water 4.carbonated beverage or beer (the CO2 gas is mixed with the liquid) 5.orange juice with pulp in it water with ice cubes in it 6.chicken noodle soup
7. sand in a desert
Separation of Matter
Elements‐ can only be broken down by nuclear reactions.
Compounds‐ can only be broken down by chemical reactions
Mixtures‐ can be broken down by physical means.
Physical Separation Methods
Filtration
http://aphschem.blogspot.com/2009_10_01_archive.html
Distillation
http://oz.plymouth.edu/~wwf/distillation.htm
Chromatography‐ physical separation based
on attraction to liquid or solid.
Paper Chromatography‐ paper is the
stationary phase and liquid is the mobile
phase.
Column Chromatography‐ beads are the
stationary phase and liquid is the mobile
phase.
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Chemical and Physical Properties Worksheet
1. Classify the following materials as heterogeneous mixtures (M), homogeneous
mixtures/solution (S), compounds (C) or elements (E).
a) air M
b) ink M
c) paper M
d) salt C
e) ethyl alcohol C
f) apple M
g) water C – M ‐ S
h) plutonium E
i) deionized water S
j) ice C
k) shaving cream M
l) paint M
m) granite M
n) 24 carat gold E
o) orange juice S
p) carbonated beverage M
q) zinc sulfate C
r) dirt M
s) river water M
t) milk S
2. Classify the following properties as chemical (C) or physical (P).
a) color P b) reactivity C c) flammability C
b) odor P e) porosity P f) stability C
g) ductility P h) solubility P i) expansion P
k) rusting C l) reacts with air C m) feel P
3. Classify the following as chemical (C) or physical (P) changes.
a) digestion of food C b) boiling water P
c) growth of a plant C d) explosion of gasoline C
e) cloud formation P f) healing a wound C
g) burning of coal C h) kicking a football P
i) contracting a muscle P j) distilling water P
k) melting silver P l) rusting iron C
m) subliming of iodine P
4. Determine the physical process to separate the following mixtures
a) ethyl alcohol and water D b) ink in a pen C
c) Sand and water F d) water and minerals F ‐ D
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Law of Conservation of Mass‐ mass can neither be gained nor lost in a chemical reaction.
o Chemical Reaction‐ creates a substance or substances known as the product(s).
o Reactants → Products
o In the complete reaction of 22.99 g of Sodium with 35.45 g of chlorine. What mass of sodium chloride will be formed?
2 Na + Cl2 → 2 NaCl
22.99 g + 35.45 g → 58.44 g NaCL
o A 12.2 g sample of X reacts with sample of Y to form 78.9 g of XY. What is the mass of Y that reacted?
X + Y → XY
12.2 g + Y → 78.9 g XY
Y = 66.7 g
Practice Problems
1. Identify the reactants and products in the following reaction.
4Fe + 3O2 2Fe2O3
Reactants = 4Fe + 3O2
Products = 2Fe2O3
2. If 112 g of Iron (Fe) reacted to produce 160 g of Iron (III) Oxide (Fe2O3), how much oxygen (O2) was
involved in the reaction? 4Fe + 3O2 2Fe2O3
112 g + (O2) 160 g
O2 = 48 g
3. When 16 grams of methane gas (CH4) combine with 64 grams of oxygen (O2), 44 grams of carbon
dioxide (CO2) form along with water. What mass of water was produced? CH4 + O2 CO2 + H2O
16 g + 64 g = 44 g + H2O
H2O = 36 g
4. When 400 grams of wood are burned, 30 grams of ash remain. Explain what may have happened to
the other 370 grams of wood.
400 g = 30 g + ? (370 g)
5. If 80.0 grams of aluminum (Al) combine with 92.5 grams of chlorine (Cl2), how many grams of
aluminum chloride will be formed? Al + 3 Cl AlCl3
80.0 g + 92.5 g = AlCl3
172.5 g = AlCl3
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Classification of Matter
Choose words from the list to fill in the blanks in the paragraphs.
Word List chemical property compound element substance
intensive property mixture physical property property
extensive property heterogeneous matter homogeneous matter
Matter that has uniform characteristics throughout is called __(1)__. Matter that has parts with different characteristics is called __(2)__. A characteristic by which a variety of matter is recognized is called a(n) __(3)__. A characteristic that depends upon the amount of matter in the sample is called a(n) __(4)__. A characteristic that does not depend upon the amount of matter is called a(n) __(5)__. A characteristic that can be observed without producing new kinds of matter is called a(n) __(6)__. A characteristic that depends on how a kind of matter changes during interactions with other kinds of matter is called a(n) __(7)__. Matter can also be classified according to the basic types of matter it contains. A simple substance that cannot be broken down into other substances by chemical means is called a(n) __(8)__. A chemical combination of different substances that retain their individual properties is called a(n) __(9)__. A physical combination of different substances that retain their individual properties is called a(n) __(10)__. Either an element or a compound may be referred to as a(n) __(11)__.
1. _homogeneous matter_
2. _heterogeneous matter
3. _ __property ________
4. ___extensive property_
5. ___intensive property_
6. ___physical property__
7. __ chemical property __
8. ___element _________
9. ___compound________
10. ___mixture__________
11. ____substance_______
12. _ heterogeneous mixture
13. ___Element___________
14. _ heterogeneous mixture
15. __________________
16. __________________
17. __________________
18. __________________
Classify each of the following as an element, compound, heterogeneous mixture, or homogeneous mixture.
12. Water
13. Carbon
14. Air
15. Table salt
16. Sugar dissolved in water
17. Homogenized milk
18. Granite
19. Oxygen
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20. Sand in water
Properties
Recall that physical properties can be observed without producing new substances. Chemical properties
describe how a substance interacts (or fails to interact) with other substances to produce new
substances. Extensive properties depend upon the amount of matter in the sample; intensive
properties do not.
Classify each of the properties listed below as extensive physical, intensive physical, or chemical.
1. Color
2. Combustibility
3. Hardness
4. Density
5. Mass
6. Melting point
7. Ductility
8. Volume
9. Failure to react with other substances
10. Odor
11. Weight
12. Malleability
13. Tendency to corrode
1. _________________
2. _________________
3. _________________
4. _________________
5. _________________
6. _________________
7. _________________
8. _________________
9. _________________
10. _________________
11. _________________
12. _________________
13. _________________
14. _________________
15. _________________
16. _________________
17. _________________
18. _________________
19. _________________
Some of the measured properties of a given substance are listed below. Write the general name describing each property. Select the names from the properties listed for Exercised 1‐13 above.
14. 15 dm3
15. Can easily be hammered into sheets.
16. 2.8 g/cm3
17. Burns when heated in the presence of O2.
18. Stinks when heated.
19. Can be scratched by a diamond.
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20. 500°C
21. Can easily be drawn into a wire.
20. _________________
21. _________________
Unit 1 Review
Complete the following calculations and report your answer with the correct number of significant
figures and with proper units.
1. 1.2 m + 2.35 m = _____________
2. 2.6538 cm x 2.1 cm = _____________
3. 5.681 dm – 2 dm = _____________
4. 3845.2 m3 25.2354 m = ____________
5. 25 cm + 3 cm = ____________
6. 1.2 m x 2 m2 = ____________
7. 859678.2354 cm – 568426.1 cm = ________
8. 5.3 m x 5.2398 m x 2 m = _____________
9. 45.25252 nm + 45.8563 nm = ____________
10. 68.23 L 38.255 L = ____________
Convert the following measurements; write your answer in standard notation or scientific notation.
Measurement Conversion (Standard Notation) Conversion (Scientific Notation)
155 cm
nm nm
155 cm
Km Km
2.77 x 10‐7 kg
mg mg
867 x 104 µL
cL cL
0.000876 Ks
ds ds
Estimate the number of significant figures in each of the following measurements. Write the measurement using Scientific Notation.
Measurement How many significant figures? Measurement in Scientific Notation
A) 10046 m
B) 500 m
C) 500. m
D) 510 m
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Round each of the measurements off to 3 significant figures. Write your answer in decimal notation
and scientific notation.
Measurement Decimal Notation Scientific Notation
A) 7534 L
B) .002346 mL
C) 16.18 cm
D) 1504 mL
Complete the following Conversions:
1. Convert 16 years to days
2. How many km/hr is 30 m/s?
3. Sally Leadfoot was pulled over on her way from Syracuse to Ithaca by an officer claiming she was speeding. The speed limit is 65 mi/hr and Sally had traveled 97 km in 102 minutes. How fast was Sally’s average speed? Does she deserve a ticket?
Physical or Chemical Properties: Indicate with a P or a C which type of change is taking place. For those labeled with a P, identify them as Intensive (I) or Extensive (E).
1. _____________ Strength
2. _____________ Color
3. _____________ Reacts with Cl
4. _____________ Volume
5. _____________ Corrodes
6. _____________ Mass
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7. _____________ Toxicity
8. _____________ Density
9. _____________ Boiling Point
10. _____________ Flammability
11. _____________ Boiling Point
12. _____________ Stability
Physical or Chemical Change? 1. ____________ glass breaking 9. ____________ mixing salt and water
2. ____________ hammering wood together 10. ____________ mixing oil and water
3. ____________ a rusting bicycle 11. ____________ water evaporating
4. ____________ melting butter 12. ____________ cutting grass
5. ____________ bleaching your hair 13. ____________ fireworks exploding
6. ____________ frying an egg 14. ____________ cutting your hair
7. ____________ squeeze oranges for juice 15. ____________ crushing a can
8. ____________ melting ice 16. ____________ boiling water
Label each process as a physical or chemical change:
a. Moth balls gradually vaporize in a closet
b. hydrofluoric acid attacks glass (used to etch
glassware)
c. Chlorine gas liquefies at ‐35 °C under normal
pressure
d. hydrogen burns in chlorine gas
Label the following as an Element (E), Compound (C), Solution (S) or Mixture (M)
a. Helium
b. Brass
c. Sodium chloride
d. Air
e. Oily water
f. Dirt
g. Wood
h. Steel
i. Iron
j. Calcium carbonate
k. Aluminum Foil
l. Glucose (a type of sugar)
Use the best physical means of separation for the following problems. 1. You are given a mixture of acetone and water, acetone has a lower boiling point than water, what method would work best to separate them?
2. Given a mixture of pepper, sand and salt, propose how you would separate the substances.
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3. You are given the task of separating ink in a pen, what method would work best to separate the
components of ink.
Answer the question using the data to support your answer.
4. Which student’s date is both accurate and precise when measuring 1.00 L of sodium chloride
solution? Explain your answer. Also include in your answer which student was the most precise.
Student: A B C D
Trial 1 1150 mL 1030 mL 850 mL 950 mL
Trial 2 1140 mL 1090 mL 1020 mL 1140 mL
Trial 3 1170 mL 1060 mL 1110 mL 1370
Matching: Match the following terms with the appropriate letter:
1. Solid _____ m. A sample that can be separated only with chemical means
2. Liquid_____
n. Anything that has mass and volume
3. Gas_____ o. An object that has a definite volume but not a definite shape
4. Matter_____ p. An object that has both definite volume and shape
5. Pure Substance_____
q. Made up of 2 or more elements
6. Compound _____ r. An object that has neither a definite shape nor volume